Practice: Counting Atoms 8. Calculating Molar Mass 4(NH_(4))_(2)SO_(3) II OIN square II OIH square II of S square It of o square

To calculate the molar mass of the compound \(4(NH_{4})_{2}SO_{3}\), we need to determine the number of atoms of each element in the compound and then multiply by the atomic mass of each element.1. **Identify the number of atoms for each element:** - : There are 2 ammonium ions ( ) in each \((NH_{4})_{2}\), and there are 2 \((NH_{4})_{2}\) units in the compound. So, there are nitrogen atoms. - : Each ammonium ion ( ) has 4 hydrogen atoms, and there are 2 ammonium ions in each \((NH_{4})_{2}\). So, there are hydrogen atoms. - : There is 1 sulfur atom in the sulfate ion ( ). - : There are 3 oxygen atoms in the sulfate ion ( ).2. **Calculate the molar mass:** - Nitrogen (N): - Hydrogen (H): - Sulfur (S): - Oxygen (O): Now, multiply the number of atoms by the atomic mass of each element: - : - : - : - : 3. **Sum the contributions:** - Total molar mass = Therefore, the molar mass of \(4(NH_{4})_{2}SO_{3}\) is .